Decomposition of Hydrogen PDF
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Added on 2021-04-21
Decomposition of Hydrogen PDF
Added on 2021-04-21
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Running head: PHYSICAL CHEMISTRY LAB REPORTPHYSICAL CHEMISTRY LAB REPORT[Author Name(s), First M. Last, Omit Titles and Degrees][Institutional Affiliation(s)]
2PHYSICAL CHEMISTRY LAB REPORTAbstractThe kinetics of the decomposition of hydrogen peroxide using manganese dioxide as the catalyst was studied at 25⁰C and 34⁰C. The findings from the experiment showed that the rate of decomposition of hydrogen peroxide increases with an increase in the amount of manganese dioxide and a rise in the temperature.IntroductionThe decomposition of hydrogen peroxide at room temperature proceeds at a very slow rate to yield water and oxygen gas. Under such conditions, there rate of collision between the moleculesof hydrogen peroxide is very slow as they have insufficient energy that is to be used in the activation of the reaction[ CITATION Pix17 \l 1033 ]. Still, the commercial hydrogen peroxide solutions among them 6% solution that is sold by beautician supply stores and the 3% hydrogen peroxide solution available in the drug stores are normally treated with stabilizers, which are at times referred to as negative catalysts[ CITATION Rob151 \l 1033 ]. These stabilizers are important in raising the activation energy for reactions involving hydrogen peroxide. In so doing, any reaction is thus further inhibited from occurring. A catalyst is a chemical substance that alters the rate of a chemical reaction and itself not consumed during the reaction. A catalyst works by lowering the activation energy that is required to initiate and maintain the reaction[ CITATION Kar12 \l 1033 ]. An example is where two hydrogen peroxide molecules react with each other forming two molecules of water and a molecule of oxygen gas as shown in the reaction below2H2O 2H2O + O2
3PHYSICAL CHEMISTRY LAB REPORTA catalyst has an immediate effect on a solution of hydrogen peroxide. The solution is observed to bubble due to the production of oxygen gas.Experimental procedure1.Mix 150 ml of distilled water, 50 ml of borate buffer solution and 10 ml of hydrogen peroxide solution in 250 ml conical flask2.Place the flask in a 298K thermostat and allow it to reach temperature equilibrium3.Add 5 ml of 0.002M KMnO4 mix well and start the stopwatch. Keep the stopwatch running throughout the experiment4.Remove a 10.0 ml sample and deliver into a conical flask containing 5-10 ml of dilute H2SO4 after 3 minutes. Record the accurate time, t when the pipette is half-empty. NOTE:When the sample is removed from the conical flask, the reaction is till occurring in the pipette. It must be quenched before analyzing. The catalyst works in alkaline solution (the borate buffer solution has a pH of about 9), so the reaction can be stopped by makingthe solution acidic[ CITATION Rob113 \l 1033 ].5.Titrate the sample with 0.002 M KMnO4 until a faint pink coloration is obtained. Record the volume, (Vt)6.Take samples after every 5 minutes for 50 minutes, or until the titre volume is around 1-2ml, whichever comes first7.Repeat the entire experiment at 308 K except take samples every 3 minutes until the titre volume is around 1-2 mlResults
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